The specific heat of ice is 2.10 kJ/kg °C, the heat of fusion for ice at 0 °C is 333.7 kJ/kg, the specific heat of water 4.186 kJ/kg °C, and the heat of vaporization of water at 100 °C is 2,256 kJ/kg. What is the final equilibrium temperature when 5.00 grams of ice at -15.0 °C is mixed with 40.0 grams of water at 75.0 °C? Multiple Choice 57.0 °C 28.3 °C 20.9 °C 18.6 °C

You mix mI = 1.2 kg of ice at TI = -19°C with mW = 3.4 kg of water at TW = 86°C in an insulated container. The specific heats of ice and water are cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively, and the latent heat of fusion for water is Lf = 3.34 × 105 J/kg. Enter an expression for the final equilibrium temperature of the mixture in terms of the defined quantities.  Hints : Heat problems involving phase changes generally need to be dealt with step by step, taking into account that when there is no temperature difference, there will be no heat transfer. In the present case, the first step might be to consider whether the ice warms to 0°C before or after the water cools to 0°C.-In an isolated system all the heat lost by any components of the system is gained by the system’s other components.-Use the relation among heat, mass, specific heat, and temperature change.-First, the ice reaches 0°C. Then it starts melting while the warmer water continues cooling. Now consider…

A 34.0-g ice cube floats in 234 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 98.2°C is dropped into the cup, and the final equilibrium temperature is 12.0°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 x 105 1/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 J/kg - °C and 387 J/kg - °C, respectively.)

A 0.200-kg mass of metal with a specific heat of 1255.8 J/kg-°C, initially at 90°C, is placed in a 0.500-kg calorimeter, with a specific heat of 418.6 J/kg-°C, initially at 20°C. The calorimeter is filled with 0.100 kg of water, initially at 20°C. The specific heat of water is 4186 J/kg-°C. What is the final temperature once the combination of metal, calorimeter, and water reach equilibrium? O 70°C 40°C 60°C O 50°C

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How much thermal energy (in J) is required to boil 2.45 kg of water at 100.0°C into steam at 135.0°C? The latent heat of vaporization of water is 2.26 ✕ 106 J/kg and the specific heat of steam is  2010  J kg · °C . HINT  J

Problem 6:   You have 4.9 kg of water in an insulated container. You add 0.95 kg of ice at -21 °C to the water and the mix reaches a final, equilibrium temperature of 11 °C. The specific heats of ice and water are 2.10 ×103 J/kg⋅C° and 4.19 ×103 J/kg⋅C°, respectively, and the latent heat of fusion for water is 3.34 ×105 J/kg.    Calculate the initial temperature of the water, in degrees Celsius.

A 500 g copper cup has an initial temperature of 250 oK. If the specific heat of copper is 385 J kg-1 oK-1 and 2.5 x 104 J of heat are transferred into it, what is the final temperature of the cup in Kelvins?

You are given 204 g of coffee (same specific heat as water) at 80.0°C (too hot to drink). In order to cool this to 60.0°C, how much ice (at 0.0°C) must be added? Ignore the heat capacity of the cup and heat exchanges with the surroundings. Specific heat capacity (15.0°C) of water is 4.186 kJ/(kg-K). The latent heat of fusion of water is 333.7 × 103 J/kg.

CALCULATION